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Atomic Structure
Atomic Structure
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A review of basic atomic structure, molar mass, and gram-mole-atom conversions.
Flashcards
33 cards
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Practice quiz
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Questions
33
Answers
1
What is the mass of 3.25 x 10
24
atoms of BeNO
3
, molar mass = 71.02 g/mol?
383.29 g
1.31 x 1025 g
2.76 x 1046 g
6.022 x 1023 g
2
Calculate the molar mass of ZnSO
4
, [Zn=65.37; S=32.06; O=16]
257.61 g/mol
453.72
113.43 g/mol
161.43 g/mol
3
How many atoms are in 4.6 mol of Ca(OH)
2
(molar mass = 74.10 g/mol)?
2.77 x 1024 atoms
74.10 atoms
7.6 x 10-24 atoms
6.022 x 1023 atoms
4
The man credited with the Law of Conservation of Matter was
Lavoisier
Proust
Dalton
Chadwick
5
Calculate the molar mass of (NH
4
)(OH): [N=14.01; H=1.01; O=16]
31.02 g/mol
35.06 g/mol
55 g/mol
70.12 g/mol
6
What is the mass of 2.5 mol of KCl {molar mass = 74.55 g/mol}?
186.38 g
196.38 atoms
186.38 mol
74.55 g
7
The number of protons in the nucleus of the atom represents the
atomic number
number of energy levels
size of the atom
atomic mass
8
Atoms that have the same atomic number but a different mass number are called
involuntary particles
icicles
isotopes
isomers
9
The negatively charged electron was discovered by
Dalton
Planck
Thomson
Rutherford
10
How many atoms are in 5.3 g of Li
2
S, molar mass = 45.94 g/mol?
5.22 x 1024 atoms
4.04 x 10-22 atoms
6.95 x 1022 atoms
6.022 x 1023 atoms
11
Neutrons were discovered to be neutrally charged by
Rutherford
Chadwick
Thomson
Bohr
12
How many moles are in 2.45 x 10
25
atoms of NaBr (molar mass = 102.89 g/mol)?
102.89
4.68 mol
10.05 mol
40.68 mol
13
The accepted Atomic Theory was developed by
Lavoisier
Bohr
Aristotle
Dalton
14
The model of the atom indicating the presence of energy levels orbiting the nucleus was done by
Bohr
Thomson
Dalton
Rutherford
15
Potassium has three naturally occuring isotopes, K-39, K-40 and K-41. Which is most abundant?
K-40
K-39
K-41
All are equally present.
16
The element Cobalt-59 has an atomic number of 27, how many electrons does it have?
32
59
86
27
17
How many atoms are in one mole of aluminum, molar mass = 26.98 g/mol?
1.62 x 1025 atoms
4.48 x 10-23 atoms
27 atoms
6.022 x 1023 atoms
18
He-4 has seven isotopes: He-3, He-4, He-5, He-6, He-7. He-8 and He-9. Which is most abundant?
He-7
He-5
He-4
He-8
19
The nucleus of the atom was discovered by
Rutherford
Dalton
Thomson
Chadwick
20
Calculate the molar mass of KMnO
4
, [K=39.1; Mn=54.94; O=16].
79 g/mol
157 g/mol
109 g/mol
226 g/mol
21
The Law of Multiple Proportions was proposed by
Lavoisier
Dalton
Aristotle
Rutherford
22
How many moles are in 4.75g of Magnesium, molar mass = 24.31 g/mol?
0.18 mol
1.97 mol
0.20 mol
2.0 mol
23
How many atoms are there in 2.3 g of NH
4
SO
2
[82.11 g/mol]?
1.69 x 1022 atoms
6.022 x 1023 atoms
2.80 x 10-2 atoms
7.33 x 1021 atoms
24
The atom is divisible into smaller particles called
neutrinos, protioids, excelesior
neutrons, electrons and protozoa
elements, compounds, molecules
electrons, protons, neutrons
25
This man determined that protons and neutrons, thus the mass, was in the nucleus of the atom.
Rutherford
Bohr
Thomson
Chadwick
26
The sum of the protons and neutrons in the nucleus of an atom is called the
average atomic mass
mass number
atomic number
isotope
27
Find the mass of 3.66 mol of N
2
, (N = 14.01 g/mol).
51.28 g/mol
102.56 g
102.56 g/mol
51.28 atoms
28
How many grams do 4.3 x 10
21
molecules of UF
6
(352.03 g/mol)?
2.12 grams
352.03 grams
2.51 grams
1.81 x 1019 grams
29
What is the molar mass of methanol (CH
3
OH) [C=12.01; H=1.01; O=16]
32.05 g/mol
29.02 g/mol
3.21 g/mol
2.90 X 1023 g/mol
30
The element Chlorine-35 has an atomic number of 17. How many neutrons does it have?
18
52
17
35
31
Matter cannot be created or destroyed is the
Law of Conservation of Matter
Atomic Theory
Law of Multiple Proportions
Law of Definite Proportions
32
A bottle of PbSO
4
(303.25 g/mol) contains 158.1 g of the compound. How many moles are there?
5.2 moles
6.022 X 1023 moles
47.943.8 3 moles
0.52 moles
33
The ratio of the masses of elements in any given compound is always the same is the
Law of Multiple Proportions
Law of Definite Proportions
Law of Conservation of Matter
Atomic Theory
